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What is the percent yield of this reaction if 750.0 g of aluminum oxide produced 256.734 g of aluminum?
Aluminum oxide, Al2O3 would produce aluminum by the following decomposition:2Al2O3 ==> 4Al + 3O2 750.0 g Al2O3 x 1 mole/101.96 g = 7.356 moles Al2O3 Theoretical yield of Al = 7.356 moles Al2O3 x 4 moles Al/2 mole Al2O3 = 14.71 moles Al Theoretical mass of Al = 14.71 moles Al x 26.98 g/mole = 396.9 g Al Percent yield = 256.734 g/396.9 g (x100%) = 64.68% yield (to 4 significant figures)
What is the equation for sulfuric acid plus aluminium III oxide?
Sulphuric Acid:- H2SO4 Aluminium Hydroxide:- Al(OH)3
Balance this equation CaOh plus H2So4 equals CaSo4 plus H2O?
The balanced equation is Ca(OH)2 + H2SO4 → CaSO4 + 2H2O.
How do you prepare 1000ppm Al solution from Al2O3?
To prepare a 1000 ppm aluminum (Al) solution from aluminum oxide (Al2O3), first calculate the amount of Al2O3 needed. Since Al2O3 contains about 53% aluminum by weight, dissolve 0.0186 grams of Al2O3 in enough water to make a final volume of 1 liter. This will yield a solution with a concentration of 1000 ppm Al. Finally, ensure thorough mixing to achieve a homogeneous solution.
Can someone help with this chemical equation K4FeC6N6 plus KMnO4 plus H2SO4 KHSO4 plus Fe2S3?
The balanced chemical equation would be K4FeC6N6 + KMnO4 + H2SO4 = KHSO4 + Fe2SO43 + MnSO4 + HNO3 + CO2 + H2O.
What is the two chemicals yield to 2 KNO2 plus H2SO4?
k2so4+hno2
Al2O3 plus HBr AlBr3 plus H2O?
Al2O3 + 6HBr = 2Albr3 + 3H2O
What does CH3OH plus H2SO4 yield?
When methanol (CH3OH) reacts with sulfuric acid (H2SO4), it forms dimethyl ether (CH3OCH3) and water (H2O) as products. This reaction is known as the dehydration of methanol.
What does H2SO4 plus KOH yield?
The reaction between sulfuric acid (H2SO4) and potassium hydroxide (KOH) will yield potassium sulfate (K2SO4) and water (H2O) as the products. This is a neutralization reaction where an acid reacts with a base to form a salt and water.
Determine the percent yield of a reaction that produces 28.65g of Fe when 50g of Fe2O3 reacts with excess Al according to the following reaction Fe2O3 plus 2Al equals Al2O3 plus 2Fe?
81.93%
What is the equation of magnesium chloride and sulfuric acid which gas is produced?
MgCl2 + H2SO4 ---> MgSO4 + 2HCl yield magnesium sulfate plus hydrogen chloride(gaz)
What is the percent yield of this reaction if 750.0 g of aluminum oxide produced 256.734 g of aluminum?
Aluminum oxide, Al2O3 would produce aluminum by the following decomposition:2Al2O3 ==> 4Al + 3O2 750.0 g Al2O3 x 1 mole/101.96 g = 7.356 moles Al2O3 Theoretical yield of Al = 7.356 moles Al2O3 x 4 moles Al/2 mole Al2O3 = 14.71 moles Al Theoretical mass of Al = 14.71 moles Al x 26.98 g/mole = 396.9 g Al Percent yield = 256.734 g/396.9 g (x100%) = 64.68% yield (to 4 significant figures)
What is the equation for sulfuric acid plus aluminium III oxide?
Sulphuric Acid:- H2SO4 Aluminium Hydroxide:- Al(OH)3
What is mn2o7 plus AL-AL2O3 plus mn blanced?
Mn2O7+Al=
What is Fe3O2 plus H2SO4?
When ferric oxide (Fe3O2) reacts with sulfuric acid (H2SO4), it forms ferric sulfate (Fe2(SO4)3) and water (H2O). The balanced equation for this reaction is: Fe3O2 + 3H2SO4 → 2Fe2(SO4)3 + 3H2O.
What is the theoretical yield of aluminum oxide if 3.40 of aluminum metal is exposed to 2.85 of oxygen?
To determine the theoretical yield of aluminum oxide, we first need to write and balance the chemical equation: 4 Al + 3 O2 -> 2 Al2O3. From the equation, we can see that 4 moles of Al reacts with 3 moles of O2 to produce 2 moles of Al2O3. Calculate the moles of Al and O2 provided, convert each to moles of Al2O3, and find the limiting reactant to determine the theoretical yield.
How many moles of aluminum oxide (Al2O3) are formed in the reaction Fe2O3 plus 2Al and rarr Al2O3 plus 2Fe?
Fe2O3 + 2Al ===> Al2O3 + 2FeIn this reaction the number of moles of Al2O3 produced is dependent on the number of moles of Fe2O3 and Al that one starts with. For every 1 mole Fe2O3 and 2 moles Al, one gets 1 moles of Al2O3.
